Domanda del libro di testo
Use the information in Table 4-2 (p. 167) to rank the following radicals in decreasing order of stability.
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Ch.4 - The Study of Chemical Reactions
Wade9th EditionOrganic ChemistryISBN: 9780135213728
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TOC.tableOfContents
- Ch.1 - Structure and Bonding107
- Ch. 2 - Acids and Bases; Functional Groups115
- Ch.3 - Structure and Stereochemistry of Alkanes100
- Ch.4 - The Study of Chemical Reactions99
- Ch.5 - Stereochemistry93
- Ch.6 - Alkyl Halides; Nucleophilic Substitution118
- Ch. 7 - Structure and Synthesis of Alkenes; Elimination158
- Ch.8 - Reactions of Alkenes171
- Ch.9 - Alkynes91
- Ch.10 - Structure and Synthesis of Alcohols143
- Ch.11 - Reactions of Alcohols104
- Ch. 12 - Infrared Spectroscopy and Mass Spectrometry22
- Ch. 13 - Nuclear Magnetic Resonance Spectroscopy45
- Ch. 14 - Ethers, Epoxides, and Thioethers72
- Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy89
- Ch. 16 - Aromatic Compounds74
- Ch. 17 - Reactions of Aromatic Compounds126
- Ch. 18 - Ketones and Aldehydes193
- Ch. 19 - Amines129
- Ch. 20 - Carboxylic Acids77
- Ch. 21 - Carboxylic Acid Derivatives141
- Ch. 22 - Condensations and Alpha Substitutions of Carbonyl Compounds175
- Ch. 23 - Carbohydrates and Nucleic Acids93
- Ch. 24 - Amino Acids, Peptides, and Proteins54
Capitolo 4, Problema 41b
Use bond-dissociation enthalpies (Table 4-2, p. 167) to calculate values of ΔH° for the following reactions.
b. CH3CH2Cl + HI → CH3CH2I + HCl
Guida verificata passo dopo passo1
Identify the bonds broken and formed in the reaction. In this case, the bonds broken are the C-Cl bond in CH3CH2Cl and the H-I bond in HI. The bonds formed are the C-I bond in CH3CH2I and the H-Cl bond in HCl.
Look up the bond-dissociation enthalpies (BDEs) for each bond in the reaction. These values can be found in Table 4-2 on page 167. For example, the BDE for a C-Cl bond, H-I bond, C-I bond, and H-Cl bond should be noted.
Calculate the total energy required to break the bonds. This is the sum of the BDEs for the bonds broken: BDE(C-Cl) + BDE(H-I).
Calculate the total energy released when the new bonds are formed. This is the sum of the BDEs for the bonds formed: BDE(C-I) + BDE(H-Cl).
Determine the overall enthalpy change (ΔH°) for the reaction by subtracting the total energy released from the total energy required: ΔH° = [BDE(C-Cl) + BDE(H-I)] - [BDE(C-I) + BDE(H-Cl)].
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Bond-Dissociation Enthalpy
Bond-dissociation enthalpy (BDE) is the energy required to break a specific bond in a molecule, resulting in the formation of two radicals. It is a crucial concept in thermochemistry, as it helps predict the stability of molecules and the energy changes during chemical reactions. BDE values are typically provided in kilojoules per mole (kJ/mol) and vary depending on the type of bond and the molecular environment.
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How to calculate enthalpy using bond dissociation energies.
Enthalpy Change (ΔH°)
Enthalpy change (ΔH°) refers to the heat content change of a system at constant pressure during a chemical reaction. It can be calculated using the bond-dissociation enthalpies of the reactants and products. The formula ΔH° = ΣBDE(reactants) - ΣBDE(products) allows chemists to determine whether a reaction is exothermic (releases heat) or endothermic (absorbs heat).
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Reaction Mechanism
A reaction mechanism describes the step-by-step sequence of elementary reactions by which overall chemical change occurs. Understanding the mechanism helps in predicting the products and the energy changes involved. In the given reaction, the mechanism involves the breaking of C-Cl and H-I bonds and the formation of C-I and H-Cl bonds, which is essential for calculating the overall enthalpy change.
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Use bond-dissociation enthalpies (Table 4-2, p. 167) to calculate values of ΔH° for the following reactions.
a. CH3—CH3 + I2 → CH3CH2I + HI
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Use bond-dissociation enthalpies (Table 4-2, p. 167) to calculate values of ΔH° for the following reactions.
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Use bond-dissociation enthalpies (Table 4-2, p. 167) to calculate values of ΔH° for the following reactions.
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